Question

NO2(g) + 7⁄2H2(g) ---> 2H2O(ℓ) + NH3(g) | ΔH° = ??? kJ |

Using the following two equations:

2NH3(g) ---> N2(g) + 3H2(g) | ΔH° = +92 kJ |

1⁄2N2(g) + 2H2O(ℓ) ---> NO2(g) + 2H2(g) |
ΔH° = +170 kJ |

Answer #1

Applying Hess’s Law, from the enthalpies of reactions,
N2(g) + 3H2(g) → 2 NH3(g) ΔH = − 91.8 kJ
O2(g) + 2H2(g) → 2H2O (g) ΔH = − 483.7 kJ
N2(g) + O2(g) → 2NO(g) ΔH = 180.6 kJ
Calculate the enthalpy change (ΔHrxn) for the reaction: 4NH3(g)
+ 5O2(g) → 4 NO (g) + 6H2O(g)

Use the following information to find ΔH°f
of gaseous HCl:
N2(g) + 3H2(g) →
2NH3(g)
ΔH°rxn = - 91.8 kJ
N2(g) + 4H2(g) +
Cl2(g) →
2NH4Cl(s)
ΔH°rxn = - 628.8 kJ
NH3(g) + HCl(g) →
NH4Cl(s)
ΔH°rxn = - 176.2 kJ

Using the Information below determine the change in enthalpy for
the following reaction:
2NO (g) + 5H2
(g)!2NH3
(g) + 2H2O
(l)
H2 (g) + 1⁄2O2 (g)!H2O (l) ΔH° = -285.8 kJ
N2 (g) + O2 (g)!2NO (l) ΔH° = +180.5 kJ
2NH3 (g)!N2 (g) + 3H2 (g)ΔH° = +92.22 kJ
a)-197.52 kJ
b)-241.7 kJ
c)-483.3 kJ
d)-659.88 kJ
e)-844.3 kJ
please show me which equation is first second and thrid and
reason why? i may be taking the wrong...

N2 (g) + 3H2 (g) → 2NH3(g) ΔH =
-92.2 kJ
What mass of ammonia is theoretically produced if the above
reaction released 183 kJ of heat?
Please show work

Calculate the ΔH∘ for this reaction using the following
thermochemical data:
CH4(g)+2O2(g)⟶CO2(g)+2H2O(l)
ΔH∘=−890.3kJ
C2H4(g)+H2(g)⟶C2H6(g)
ΔH∘=−136.3kJ
2H2(g)+O2(g)⟶2H2O(l)
ΔH∘=−571.6kJ
2C2H6(g)+7O2(g)⟶4CO2(g)+6H2O(l)

From the enthalpies of reaction
2H2(g)+O2(g)→2H2O(g)ΔH=−483.6kJ3O2(g)→2O3(g)ΔH=+284.6kJ calculate
the heat of the reaction 3H2(g)+O3(g)→3H2O(g) Express your answer
using four significant figures. I have no idea how to approach this
problem.

Using the information below determine the change in enthalpy for
the following reaction:
2NO(g) + 5 H2(g) → 2NH3(g) +
2H2O(l)
H2(g) + ½ O2(g) →
H2O(l)
∆H°= -285.8kJ
N2(g) + O2(g) →
2NO(g)
∆H°= +180.5 kJ
2NH3(g) → N2(g) +
3H2(g)
∆H°= + 92.22 kJ
please explain step by step! thanks!

Please solve step by step for Part D
Consider the Haber synthesis of gaseous NH3
(ΔH∘f=−46.1kJ/mol ;ΔG∘f=−16.5kJ/mol) :
N2(g)+3H2(g)→2NH3(g)
Part A
Use only these data to calculate ΔH∘ and ΔS∘
for the reaction at 25 ∘C.
Express your answers using three significant figures separated
by a comma.
ΔH∘, ΔS∘ =
-92.2,-199
kJ, J/K
Part D. What are the equilibrium constants Kp
and Kc for the reaction at 370 K ? Assume that
ΔH∘ and ΔS∘ are independent of
temperature.
Express...

#5.133
A mixture of NH3(g) and N2H4(g) is placed in a
sealed container at 320 K . The total pressure is 0.53 bar . The
container is heated to 1200 K at which time both substances
decompose completely according to the equations
2NH3(g)→N2(g)+3H2(g) ;
N2H4(g)→N2(g)+2H2(g) . After
decomposition is complete the total pressure at 1200 K is found to
be 4.5 bar.
Find the percent (by volume) of N2H4(g) in the original
mixture. (Assume two significant figures for the temperature.)

1. The equilibrium constant, Kp, for the following reaction is
4.55×10-5 at 723 K.
N2(g) + 3H2(g) 2NH3(g)
If ΔH° for this reaction is -111 kJ, what is the value of Kp at
839 K?
Kp=
2. The equilibrium constant, Kp, for the following
reaction is 0.110 at 298 K.
NH4HS(s)
NH3(g) +
H2S(g)
If ΔH° for this reaction is 92.7 kJ, what is the
value of Kp at 393 K?
Kp=

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